Lead(II) iodide is a poorly water soluble solid compound. Its Ksp is 1.4 x 10* (at 25°C). What is the solubility of lead(1I) iodide in water at 25°C ? (in units of molarity) Write the Køp expression first. Lead(II) iodide is Pblz. The molar mass of lead(1I) iodide is 461 g/mol. How much lead(II) iodide, in grams, will dissolve in 100 mL of water at 25°C? (this is the nominal solubility of lead(II) iodide)

The Kp of manganese(II) hydroxide, Mn(OH)2, is 2.00 x 10-13. Calculate the solubility of this compound in grams per liter. 3.68 x10-5

Predict what will happen when you add 280 mg of BaF2 (175.3 g/mol) to 500 mL of water (Ksp of BaF2 is 1.84 x 10-7). QK, all 280 mg will dissolve. Q>K, some of the CaCO3 will precipitate. Q=K, the solution will be at perfect equilibrium and Luke will have finally brought balance to the force.

Solid cobalt(II) nitrate is slowly added to 50.0 mL of a 0.0541 M sodium hydroxide solution. The concentration of cobalt(II) ion required to just initiate precipitation is  M. (Assume that Ksp (Co(OH)2)= 2.5 x 10^-16).

The solubility of lead(II) chloride, PbCl2 (MM: 278.1 g/mol), in water at 60 °C is 1.94 g/L.  Ksp for lead(II) chloride = 1.37×10^-6 a) Using your value of Ksp, what is the molar solubility of lead(II) chloride in a 0.102 M solution of NaCl?

What is the molar solubility (in M to two decimal places) of cadmium carbonate in water (at 25 °C)? Ksp = 5.2 × 10–12

The Ksp of manganese(II) carbonate, MNCO3, is 2.42 × 10-11. Calculate the solubility of this compound in g/L. L

The solubility-product constants, Kp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Substance Кар FeCO3 2.10 x 10-11 CdCO3 1.80 x 10-14 Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.03x10-2 M Fe2+ and 1.52x10-2 MCd2+. What concentration of CO² is need to initiate precipitation? Neglect any volume changes during the addition. Express your answer with the appropriate units. ▸ View Available Hint(s) [CO32] = Value Units Submit Part B Complete previous part(s) Part C Complete previous part(s) Provide Feedback ? Next >

A 100.0 mL mixture is made of water and 1.0 g of silver chloride, AgCl.  What does this solution look like, and what mass of silver chloride is in solution?  The molar solubility of AgCl = 1.3x10-5, and the molar mass of AgCl = 143.32 g/mol.   A.1.9x10-4 (Clump of AgCl undissolved in beaker of water) B. 1.3x10-5 (Clump of AgCl undissolved in beaker of water)

Calculate the solubility (in g/L) of CaSO, (s) in 0.300 M Na, SO,(aq) at 25°C. The K5p of CaSO, is 4.93 x 10-5. The molar mass of CaSO4 is 136.14 g mol-l. solubility: g/L